Use the tabulated electrode potentials to calculate K for the oxidation of iron by H++ (at 25°C): 2Fe(s)+6H+(aq)→2Fe3

An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.19 M FeSO4 solution and a copper electrode in 1.00 L of 8.80 × 10-² M CuSO4 solution. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction ¯(aq) + 2e¯ ⇒ Fe(s) Cu²+ (aq) + 2e¯¯ ≈ Cu(s) Fe²+ Standard Potential, E° (V) -0.41 = 0.34 a. What is the initial voltage of this cell when it is properly constructed? Initial voltage 2+ b. Calculate the final concentration of Cu²+ in this cell if it is allowed to produce an average current of 1.78 amp for 241 s. Final concentration of Cu²+ M

The standard cell potential for reaction, Fe(s) + Cu²⁺(aq) → Fe²⁺(aq) + Cu(s) is E⁰ = 0.17V. What is the cell potential if [Cu²⁺(aq)] = 1.0M and [ Fe²⁺(aq] = 0.1M

Consider a galvanic cell based on the reaction   2 Fe2+ (aq)     +   Cl2 (g)   ------------>2 Fe3+ (g)    +          2Cl- (aq)   Calculate the cell potential at 25oC when [Fe2+  ] =1.0 M,  [Fe3+ ] = 1.0 x 10-3 M,  [Cl- ] = 3.0 x 10-3 M and PCl2 = 0.50 atm.

The electrochemical cell Cu|Cu 2+||Al 3+|Al has a potential of –1.997 V under standard conditions. What is the standard reduction potential for the reaction of Al 3+ Al?

Mg(s) + Fe²+(aq) → Mg²+ (aq) + Fe(s) The galvanic cell described above has a standard cell potential of 1.93 V. The standard reduction potential of Mg2+ corresponding to the half-reaction Mg2+ (aq) + 2e- Mg(s) is -2.37 V. Calculate the standard reduction potential of iron(II). EFe²+ = V

I need to find standard cell potential, the non-standard cell potential, using [Au^+]= 0.0015M and [Fe^3+]= 0.033M.  I need to calculate Gibb's free energy and equilibrium constant, K.  Is the reaction spontaneous or nonspontaneous?  Are reactants or products favored at equilibrium under non-standard conditions?

3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) Determine the cell potential for the reaction at a pH of 4.0 ( you will need to use the Nernst equation) Assume that all concentrations, other than that of H+, are standard.

[Fe3+]= 2.0×10−3 M; [Mg2+]= 3.15 M   Express your answer in units of volts.

A quantity of electricity equal to 6.95 × 104 C passes through an electrolytic cell that contains a solution of Sn4+(aq) ions. Compute the maximum chemical amount, in moles, of Sn(s) that can be deposited at the cathode.